Correct order of bond angle is

Options

A. (A)`(*CH_(3))gt(*CH_(3))`
B. (B)`CH_(3)^(-)gtCH_(3)^(+)`
C. (C)`CH_(4)gtCF_(4)`
D. (D)`CH_(4)gt(*CH_(3))`

Explanation

To determine the correct order of bond angles among the given molecules, we will analyze the bond angles based on the molecular geometry and the presence of lone pairs or radicals.

### Step-by-Step Solution:

1. **Identify the Molecules and Their Structures**:
- We have several molecules to compare: CH3-, CH3+, CH4, CF4, and CH3 radical.

2. **Analyze CH3- (Methyl Anion)**:
- CH3- has a tetrahedral geometry but with one lone pair on the carbon atom. The presence of the lone pair will cause the bond angles to be slightly less than the ideal tetrahedral angle of 109.5° due to lone pair-bond pair repulsion. Therefore, the bond angle in CH3- is less than 109.5°.

3. **Analyze CH3+ (Methyl Cation)**:
- CH3+ is a carbocation with a trigonal planar geometry. The bond angles in this structure are approximately 120° due to sp² hybridization. Therefore, the bond angle in CH3+ is 120°.

4. **Analyze CH4 (Methane)**:
- CH4 has a perfect tetrahedral geometry with bond angles of 109.5° since there are no lone pairs to affect the angles.

5. **Analyze CF4 (Carbon Tetrafluoride)**:
- CF4 also has a tetrahedral geometry with bond angles of 109.5°, similar to CH4, as it has no lone pairs.

6. **Analyze CH3 Radical**:
- The CH3 radical has a tetrahedral geometry as well, but due to the presence of one unpaired electron, the bond angles will be slightly less than 109.5° due to increased electron-electron repulsion.

7. **Compare the Bond Angles**:
- CH3- < CH3 radical < CH4 = CF4 < CH3+
- Therefore, the correct order of bond angles from smallest to largest is:
- CH3- < CH3 radical < CH4 = CF4 < CH3+

### Conclusion:
The correct order of bond angles is:
- CH3- < CH3 radical < CH4 = CF4 < CH3+